Can you help me with these questions ???? An impure sample containing phosphoric

Question

Can you help me with these questions ???? An impure sample containing phosphoric acid was completely neutralized with strong base. The titration required 90.0 ml of 0.222 M NaOH solution. If the formula for phosphoric acid is H_3PO_4, calculate the equivalent weight of the acid. How many moles of protons were titrated? How many moles of H_3 PO_4 were titrated? How many grams of H_3 PO_4 were titrated? If the impure sample weighed 8.45 g, what is percentage of phosphoric acid contained in the sample?

Explanation / Answer

1)

a)
molar mass of H3PO4 = 98 g/mol
it has 3 proton

equivalent weight = 98/3 g/equiv

b)
moles of proton = moles of OH-
= M*V
= 0.222 M * 0.090 L
= 0.01998

c)
moles of H3PO4 = 0.01998/3 = 0.00666 mol

d)
mass of H3PO4 = moles of H3PO4 * molar mass
= 0.00666 mol * 98 g/mol
= 0.653 g

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